A solution is made by adding 0.380 gg Ca(OH)2(s)Ca(OH)2(s), 50.0 mLmL of 1.45 MM HNO3HNO3, and enough water to make a final volume of 75.0 mLmL. Part A Assuming that all of the solid dissolves, what is the pH of the final solution

pH of the final solution is 0.08

Explanation:

To calculate the moles, we use the equation:

a) moles of =

b) To calculate the number of moles for given molarity, we use the equation:

Molarity of solution = 1.45 M

Volume of solution = 50.0 mL

1 mole of reacts with 2 moles of

Thus 0.0051 moles of reacts with = moles of

Moles of left = (0.0725-0.0102) = 0.0623

Thus 0.0623 moles of are left in 75.0 ml of solution

Molarity of

pH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

Thus pH of the final solution is 0.08

b. is the answer hoped i